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Chapter 3: Problem 45

Why is the atomic mass scale also called the relative atomic mass scale?

Short Answer

Expert verified
The atomic mass scale is called the "relative atomic mass scale" because it measures the atomic masses of elements in comparison to the mass of a carbon-12 atom, which is the reference element. The term "relative" emphasizes that atomic masses are a dimensionless comparison rather than an absolute measurement of an atom's mass.

Step by step solution

01

Understanding Atomic Mass:

Atomic mass is the measure of the mass of an atom of an element. Atomic masses are usually expressed in atomic mass units (amu), where 1 amu is equal to one twelfth of the mass of a carbon-12 atom. It is calculated as the weighted average mass of the naturally occurring isotopes of the element, taking into account the abundance of each isotope.
02

Basis of the Atomic Mass Scale:

In the atomic mass scale, the reference element chosen to define the atomic mass unit is the carbon-12 isotope. It means that the atomic mass of a carbon-12 atom is exactly 12 amu. The atomic masses of other elements are measured relative to the mass of a carbon-12 atom. Therefore, the atomic mass scale is essentially a comparison of the masses of other elements to the mass of a carbon-12 atom.
03

Relative Atomic Mass and its Significance:

Since the atomic masses of elements are determined in comparison to a reference element (carbon-12), the atomic mass values are considered as dimensionless quantities. This relative comparison gives rise to the term "relative atomic mass." The use of the term "relative" emphasizes the fact that atomic masses are a comparison rather than an absolute measurement of an atom's mass.
04

Conclusion:

The atomic mass scale is called the "relative atomic mass scale" because the atomic masses of elements are determined in comparison to a reference element, which is the carbon-12 isotope. The atomic masses of other elements are expressed relative to the mass of a carbon-12 atom, making the atomic mass scale a dimensionless comparison of the atomic masses.

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Most popular questions from this chapter

The element nitrogen has only two naturally occurring isotopes: \({ }^{14} \mathrm{~N}\) with a mass of \(14.00308\) amu and an abundance of \(99.635 \%\) and \({ }^{15} \mathrm{~N}\) with a mass of \(15.00011\) amu and an abundance of \(0.3650 \%\). Calculate the atomic mass of nitrogen.

A student says that it is possible for an atom's second ionization energy to be zero because all the work was done creating a cation with the first jonization energy. Is this student right or wrong? Explain.

Scandium (Sc) is a metal that tends to lose three electrons. Copper (Cu) and zinc \((Z n)\) are also metals that tend to lose one and two electrons, respectively. Knowing this, explain why the first group in the transition metals is numbered IIIB, whereas the last two groups in the transition series are numbered IB and IIB, respectively.

Metals are excellent conductors of electricity. Nonmetals are poor conductors of electricity and are called insulators. Some elements have the ability to conduct electricity roughly between that of metals and nonmetals. Give some examples of these elements, and name the class they belong to.

The mass number of a \(2+\) cation is 56 , and its atomic number is 26 . The ion contains how many protons, electrons, and neutrons?
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